To find the longest wavelength of photon that can break this bond, we need to use the equation for the energy of a photon, which is E = hc/λ, where E is the energy, h is Planck's constant, c is the speed of light, and λ is the wavelength.

Step 1: Convert the bond dissociation energy from kJ/mole to J/photon.

1 mole of photons is Avogadro's number (6.022 x 10^23 photons).

So, 200 kJ/mole = 200,000 J/mole = 200,000 J / 6.022 x 10^23 photons = 3.32 x 10^-19 J/photon.

Step 2: Substitute the values into the equation E = hc/λ.

We know that h = 6.626 x 10^-34 J.s and c = 3.00 x 10^8 m/s.

So, 3.32 x 10^-19 J = (6.626 x 10^-34 J.s)(3.00 x 10^8 m/s) / λ.

Step 3: Solve for λ.

λ = (6.626 x 10^-34 J.s)(3.00 x 10^8 m/s) / 3.32 x 10^-19 J = 5.99 x 10^-7 m or 599 nm.

So, the longest wavelength of photon that can break this bond is approximately 599 nm.

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To find the longest wavelength of photon that can break this bond, we need to use the equation for the energy of a photon, which is E = hc/λ, where E is the energy, h is Planck's constant, c is the speed of light, and λ is the wavelength.

Step 1: Convert the bond dissociation energy from kJ/mole to J/photon.

1 mole of photons is Avogadro's number (6.022 x 10^23 photons).

So, 200 kJ/mole = 200,000 J/mole = 200,000 J / 6.022 x 10^23 photons = 3.32 x 10^-19 J/photon.

Step 2: Substitute the values into the equation E = hc/λ.

We know that h = 6.626 x 10^-34 J.s and c = 3.00 x 10^8 m/s.

So, 3.32 x 10^-19 J = (6.626 x 10^-34 J.s)(3.00 x 10^8 m/s) / λ.

Step 3: Solve for λ.

λ = (6.626 x 10^-34 J.s)(3.00 x 10^8 m/s) / 3.32 x 10^-19 J = 5.99 x 10^-7 m or 599 nm.

So, the longest wavelength of photon that can break this bond is approximately 599 nm.

Knowee AI · Accepted Answer

To find the longest wavelength of photon that can break this bond, we need to use the equation for the energy of a photon, which is E = hc/λ, where E is the energy, h is Planck's constant, c is the speed of light, and λ is the wavelength.

Step 1: Convert the bond dissociation energy from kJ/mole to J/photon.

1 mole of photons is Avogadro's number (6.022 x 10^23 photons).

So, 200 kJ/mole = 200,000 J/mole = 200,000 J / 6.022 x 10^23 photons = 3.32 x 10^-19 J/photon.

Step 2: Substitute the values into the equation E = hc/λ.

We know that h = 6.626 x 10^-34 J.s and c = 3.00 x 10^8 m/s.

So, 3.32 x 10^-19 J = (6.626 x 10^-34 J.s)(3.00 x 10^8 m/s) / λ.

Step 3: Solve for λ.

λ = (6.626 x 10^-34 J.s)(3.00 x 10^8 m/s) / 3.32 x 10^-19 J = 5.99 x 10^-7 m or 599 nm.

So, the longest wavelength of photon that can break this bond is approximately 599 nm.

Bond dissociation on energy of Br2 is 200 kJ/mole. The longest wavelength of photon that can breakthis bond would be

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